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The rate of reaction in terms of the "rate law expression" includes the rate constant (kk), the concentration of the reactants, and the orders of the reaction with respect to the different reactants. Consider the following reaction: A+B→C+DA+B→C+D The initial concentrations of the reactants AA and BB are 0.200 MM and 0.350 MM, respectively. The rate of reaction is 0.060 M⋅s−1M⋅s−1, and the orders of the reaction, with respect to reactants AA and BB, are 1 and 2, respectively. Determine the rate constant (kk) for the reaction using the rate law. Express your answer in M−2⋅s−1M−2⋅s−1 to three significant figures.

Respuesta :

sebassandin

Answer:

[tex]k=2.45M^{-2}s^{-1}[/tex]

Explanation:

Hello.

In this case, considering the given specific orders of reaction, we can write the rate law as:

[tex]r=k[A][B]^2[/tex]

Thus, considering the concentrations of A and B to be 0.200 M and 0.350 M respectively and a rate of 0.060 M/s, the rate constant turns out:

[tex]k=\frac{r}{[A][B]^2}\\ \\k=\frac{0.060M/s}{(0.200M)(0.350M)^2} \\\\k=2.45M^{-2}s^{-1}[/tex]

This is what we know as a third-order reaction since the specific orders both add to 3.

Best regards.

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